40) Calculate the pH of a solution prepared by mixing 0.0870 mol of chloroacetic acid plus 0.0250 mol of sodium chloroacetate in1.00 L of water.First do the calculation by assuming that the concentrations of HA and A- equal their formal concentrations. The pK, ofchloroacetic acid is 2.865.pH =2.323Then do the calculation with [HA] and [A-] from Equations 9-21 and 9-22.[HA] = FHA – [H*]+ [OH¯](9-21)[A] = FA- + [H*] – [OH-](9-22)8.54 x103pH =IncorrectUsing first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all thefollowing compounds in one beaker containing a total volume of 1.00 L: 0.250 mol CICH,CO,H, 0.090 mol CICH,CO, Na,0.080 mol HNO,, and 0.080 mol Ca(OH),. Ca(OH), provides 2 OH-.pH =2.865

pH =pKa + log[Conjugate Base][acid] pH =pKa + log[Sodium Chloroacetate][Chloro acetic acid] pH…

Calculate the pH of a solution prepared by mixing 0.0870 mol of chloroacetic acid plus 0.0250 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A- equal their formal concentrations. The pK, of chloroacetic acid is 2.865. pH = 2.323 Then do the calculation with [HA] and [A-] from Equations 9-21 and 9-22. [HAJ = FHA – [H*]+ [OH¯] (9-21) [A-] = FA + [H*]- [OH-] (9-22)

Calculate the pH of a solution prepared by mixing 0.0870 mol of chloroacetic acid plus 0.0250 mol of sodium chloroacetate in 1.00 L of water. First do the calculation by assuming that the concentrations of HA and A- equal their formal concentrations. The pK, of chloroacetic acid is 2.865. pH = 2.323 Then do the calculation with [HA] and [A-] from Equations 9-21 and 9-22. [HAJ = FHA – [H]+ [OH¯] (9-21) [A-] = FA + [H]- [OH-] (9-22)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 107AP

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